CHEM 2301 Chapter Notes - Chapter 1: Orbital Hybridisation, Valence Electron, Sigma Bond
Document Summary
Chem 2301 notes ch 1: structure and bonding. Anion: negatively charged ion from gained electrons. Isotopes: 2 atoms of same element but different # of neutrons and different mass #. Orbitals: subshells in atoms with high electron density. 4 kinds include: s, p, d, & f. each orbital can hold maximum of 2 electrons: s orbital: sphere shaped electron density. Lowest energy level: p orbital: dumbbell shape. Higher energy than s orbital because electrons are further from nucleus (filled after s is complete). Core electrons: electrons in the inner shell of orbitals. Valence electrons: participate in chemical reactions because they are in outer shell and held loosely by the nucleus compared to core electrons. Group # of the second row periodic table elements = # of valence electrons. Formal charge= # valence electrons - # electrons atom owns (bonds + all lone pairs) ** lone pair= 2 owned electrons, while a bond= 1 owned electron.
